Answer:
The correct option is H₂O is an acid and OH⁻ is its conjugate base.
Explanation:
According to the Bronsted-Lowry theory, an acid is a substance capable of yielding a hydrogen ion while a base is a species capable of accepting a hydrogen ion.
A conjugated acid-base pair is a pair of chemical species capable of transforming into each other by exchange of a proton. That is, a conjugated acid is the species that forms after the base accepts a proton. In contrast, a conjugate base is the species that forms after an acid donates its proton.
So, in this case water acts as an acid, yielding a proton to HCO₃⁻, which in turn acts as a base.
The correct option is H₂O is an acid and OH⁻ is its conjugate base.
H₂O acts as an acid and OH⁻ is its conjugate base. The correct option is d) H₂O is an acid and OH⁻ is its conjugate base
An acid can be defined as any substance that can donate a proton .
A base can be defined as any substance that can accept a proton.
When an acid donates a proton, the acid changes into a base. That base is referred to as the acid conjugate base; and
When a base accepts a proton, an acid is formed. That acid is referred to as the base conjugate acid.
In the given reaction,
HCO₃⁻(aq) + H₂O(aq) → H₂CO₃(aq) + OH⁻(aq)
H₂O donates a proton to HCO₃⁻, therefore H₂O acts as an acid.
When H₂O loses a proton, OH⁻ is formed, therefore OH⁻ is its conjugate base.
Hence, H₂O acts as an acid and OH⁻ is its conjugate base. The correct option is d) H₂O is an acid and OH⁻ is its conjugate base.
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